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- 1. Multiple Choice
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each element....
decreases
increases
remains the same
none of the above
- 2. Multiple Choice
Which atom has the largest atomic radius?
potassium
rubidium
francium
cesium
- 3. Multiple Choice
As you move down the periodic table atoms get bigger. This is because ____________.
The atoms have more mass.
The atoms have more protons.
The atoms have more energy levels
The atoms have more nuetrons
- 4. Multiple Choice
As you move across the periodic table atoms tend to get smaller because, ______________.
the atoms have more mass.
the atoms have less mass
the atoms have more protons.
the atoms have less electrons.
- 5. Multiple ChoiceAtoms that have a high electronegativity, _______________.give up their electrons more easily.hold on to their electrons more tightly.have more electron shells.
- 6. Multiple ChoiceIonization energy is...the energy required to add an electron to a specific atomhow much energy it takes to remove an electron from an atomthe energy required to shield the outer electrons from the nucleusa measure of the ability of an atom to attract electrons
- 7. Multiple Choice
Metals have the largest -
atomic radius and electronegativity
electronegativity and ionization energy
atomic radius only
ionization energy and atomic radius
- 8. Multiple Choice
The element with the largest electronegativity in the halogens is -
At
F
Cl
Br
- 9. Multiple Choice
The element with the lowest electronegativity in Period 3 is -
Na
Cl
Ar
Mg
- 10. Multiple Choice
The electronegativity of Cl is the highest in Period 3. Why?
Cl is the largest and has the greatest effective nuclear charge
Cl is the smallest and has the lowest effective nuclear charge
Cl is the largest and has the lowest effective nuclear charge
Cl is the smallest and has the greatest effective nuclear charge
- 11. Multiple Choice
The element with the smallest ionization energy in Period 6 is -
Rn
Cs
Os
Tm
- 12. Multiple Choice
As we go from the left side to the right side on the periodic table, electronegativity...
Increases
Decreases
Remains constant
- 13. Multiple Choice
The tendency of an atom to attract electrons and acquire a negative charge
electronegativity
charge
bonding ability
electron configuration
- 14. Multiple ChoiceVertical columns of elements (families) on the periodic table with similar valence electron configurations and similar propertiesgroupsperiodsquadrantsrows
- 15. Multiple Choice
An electron that resides in the outermost shell, or principal quantum level, of an atom
periodic trend
electron shell
ionic radius
valence electron
- 16. Multiple Choice
Which has the greater EN (electronegativity)
Cl or Al?
Cl
Al
- 17. Multiple ChoiceWhich has the greater EN:
H or F?HF - 18. Multiple Choice
The term that is related to the number of protons is
Ionization energy
Electronegativity
Nuclear Charge
Shielding effect
- 19. Multiple ChoiceElectronegativity __________ from left to right within a period and __________ from top to bottom within a group.decreases, increasesincreases, increasesincreases, decreasesstays the same, increases
- 20. Multiple ChoiceWho was the first to organize the periodic table based on increasing atomic massMendeleevMoseleyNewtonSchrodinger
- 21. Multiple ChoiceGroup 1A, very reactive in waterTransition MetalsAlkali MetalsAlkaline Earth Metals
- 22. Multiple ChoiceGroup 2A, includes Mg & CaAlkali MetalsAlkaline Earth MetalsTransition Metals
- 23. Multiple ChoiceWhich of the following has the highest Ionization energy?LiKClCa
- 24. Multiple ChoiceAtomic radius generally increases as we move __________.down a group and from right to left across a periodup a group and from left to right across a perioddown a group and from left to right across a periodup a group and from right to left across a period
- 25. Multiple Choice
This trend illustrates the attraction of an atom for electrons.
Atomic Size
Metallic Character
Electronegativity
Ionization Energy
- 26. Multiple Choice
This trend illustrates the energy associated with the removal of an electron from an atom.
Atomic Size
Metallic Character
Electronegativity
Ionization Energy
- 27. Multiple Choice
In general, which group will have the overall highest electronegativity values?
Noble Gases
Halogens
Alkali Metals
Alkaline Earth Metals
- 28. Multiple Choice
Which element will have the lowest ionization energy?
Na
Cl
K
Br
- 29. Multiple ChoiceAccording to the diagram Li will form a ____________ with a _________ charge.cation, +1anion, +1cation, -1anion, -1
- 30. Multiple ChoiceThe trend of ionization energy seen on the periodic table is increase across a period and up a column. As seen in the image. Which would have a greater ionization energy, K or Na?KNa
- 31. Multiple ChoiceWhich element would use less energy to remove an electron from its orbital? P or ArPAr
- 32. Multiple ChoiceRank in order of lowest to highest ionization energy: Si, Mg, SS, Mg, SiMg, Si, SSi, Mg, S
- 33. Multiple ChoicePut the following in order of increasing ionization energy:Neon, Lithium, CarbonLithium, Carbon, NeonCarbon, Lithium, NeonNeon, Carbon, LithiumLithium, Neon, Carbon
- 34. Multiple ChoiceWhich of the following would produce an anion?CaAlKF
- 35. Multiple Choice
A horizontal row on the periodic table is called a ______________
Period
Group
- 36. Multiple Choice
Which group of elements has the lowest ionization energy?
Group 1
Group 2
Group 3
Group 4
- 37. Multiple Choice
Order the following in decreasing electronegativity value:
Ga, Fe, As, K
Ga, Fe, As, K
K, As, Fe, Ga
As, Ga, Fe, K
Fe, K, Ga, As
- 38. Multiple ChoiceWhich of the following is true?Electronegativity increases from right to left across a periodAtomic Radii decrease from left to right across a periodIonization energy increases from left to right across a periodOxidation numbers increase from right to left across a period
- 39. Multiple ChoiceWhich of the following is true?Electronegativity increases up a groupAtomic Radii increases up a groupIonization energy increases down a groupOxidation numbers increase down a group
- 40. Multiple Choice
Our modern Periodic Table is organized by increasing....
oxidation numbers
average atomic mass
atomic number
alphabetical order
- 41. Multiple Choice
The table shows the first ionization energy and atomic radius of several elements. Which of the following best helps to explain the deviation of the first ionization energy of oxygen from the overall trend?
The atomic radius of oxygen is greater than the atomic radius of fluorine.
The atomic radius of oxygen is less than the atomic radius of nitrogen.
There is repulsion between paired electrons in oxygen’s 2p orbitals.
There is attraction between paired electrons in oxygen’s 2p orbitals.
- 42. Multiple Choice
The ionization energies for element X are listed in the table on the right. On the basis of the data, element X is most likely to be
Be
B
C
F
- 43. Multiple Choice
For element X represented above, which of the following is the most likely explanation for the large difference between the second and third ionization energies?
The effective nuclear charge decreases with successive ionizations.
The shielding of outer electrons increases with successive ionizations.
The electron removed during the third ionization is, on average, much closer to the nucleus than the first two electrons removed were.
The ionic radius increases with successive ionizations.
- 44. Multiple Choice
Which of these has the greatest ionic radius?
potassium
aluminum
carbon
oxygen
- 45. Multiple ChoiceWhat is the term that describes the adding of energy levels as you move down the periodic table?multiplyingShieldinggrowinglayering
- 46. Multiple Choice
Which of the following elements have the smallest ionic Radius?
Oxygen
Selenium
Sulfur
Tellurium
- 47. Multiple ChoiceThe bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?They are in the same period with W being furthest left.They are in the same period with W being furthest right.They are in the same group with W being furthest to the bottom.They are in a diagonal line with W being at the bottom right.
- 48. Multiple ChoiceWhich of the following is true for alkaline earth metals as their atomic number increases?The atomic radius decreases.Ionization energy decreases.The number of valence electrons increases.The Coulombic attraction increases.
- 49. Multiple ChoiceWhich of the following sequences corresponds to a correct trend in ionization energy?Cl > S > P > AlSr > Ca > Mg > BeRb > K > Na > LiRb > Sr > I > Xe
- 50. Multiple Choice
The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?
The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
The ionization energy increases gradually as you move right across a period because you are adding more protons.
The ionization energy increases when the valence electrons are more attracted to the nucleus.
- 51. Multiple Choice
Across a period from left to right, the effective nuclear charge __________ and ionization energy_____________.
increases
decreases
increases
increases
decreases
decreases
decreases
increases
- 52. Multiple Choice
Which of the following elements has the highest electronegativity?
Ca
Mg
Ba
Sr
- 53. Multiple Choice
For which of the following elements would you expect a large jump between IE1 and IE2?
Na
Fe
Ca
F
- 54. Multiple Choice
Which of the following elements has the smallest first ionization energy?
Na
Cl
Cs
I
- 55. Multiple Choice
Nuclear charge ________ across a period
Increases
Decreases
Stays the same
- 56. Multiple ChoiceHow many shielding electrons does carbon have? (hint: write its configuration first)1234
- 57. Multiple ChoiceAs you go across a period, the amount of shielding...Increasesdecreasesstays the same
- 58. Multiple ChoiceAs you move across a period, the effective nuclear charge...increasesdecreasesstays the same
- 59. Multiple ChoiceWhich of the following elements has the highest effective nuclear charge?IndiumAntimonytelleriumTin
- 60. Multiple ChoiceIn the following configuration, which electrons are the shielding electrons? 1s2 2s2 2p6 3s2 3p41s2 2s2 2p63s2 3p41s2 2s22s2 2p6 3s2 3p4
- 61. Multiple ChoiceShielding electrons are:Electrons in the highest energy levelElectrons in the lower energy levelsElectrons that just come and go - they don't stay with the atomElectrons that are excited
- 62. Multiple ChoiceThe effective nuclear charge is _____ the actual nuclear chargethe same asless thangreater than
- 63. Multiple Choice
Effective nuclear charge ___ down a group of elements
Increases
Decreases
Stays the same
- 64. Multiple Choice
How many valence electrons are there in the element with the following ionization energies?
755 kJ/mol , 1230 kJ/mol , 2283 kJ/mol , 4322 kJ/mol , 9763 kJ/mol, 22925kJ/mol, 31170 kJ/mol
2
3
4
5
6
- 65. Multiple Choice
The reactivity of group 1 metals can best be explained by;
Their overall high electronegativity
Their overall high effective nuclear charge
The instability of their nuclei
Their overall low ionization energy
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